When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7 o C was measured for the beaker and its contents (Expt.1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant ( - 57.0 k J m o l - 1 ) , this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL o

Step-by-step solution

Let the heat capacity of insulated beaker be C. Mass of aqueous content in Expt. 1 = 100 + 100 × 1 = 200 g ⇒ T o t a l h e a t c a p a c i t y = C + 200 × 4.2 J / K Moles of acid, base neutralized in Expt. 1 = 1 × 0.1 = 0.1 ⇒ Heat absorbed in Expt. 1 = 0.1 × 57 = 5.7 k J ⇒ 5.7 × 1000 = C + 200 × 4.2 × Δ T ⇒ 5.7 × 1000 = C + 200 + 4.2 × 5.7 ⇒ C + 200 × 4.2 = 1000 In Second experiment n C H 3 C O O H = 0.2 , n N a O H = 0.1 Total mass of aqueous content = 200 g ⇒ Total heat capacity = C + 200 × 4.2 = 1000 ⇒ Heat rele